Warm UP - Practice Write or name the following compounds Ca(OH)2 7) Sr3(PO3)2 8) MgF2 9) LiBr 10) Mn2O7 Iron (III) Nitrite 2) Sodium Chloride 3) Silver Phosphate 4) Cadmium Oxide 5) Aluminum Phosphide

Practice 2) MgSO4 • 7 H2O 3) CrBr3• 6H2O 4) Pb(ClO3)2 • 3H2O 1) MnBr2• 4 H2O 2) MgSO4 • 7 H2O 3) CrBr3• 6H2O 4) Pb(ClO3)2 • 3H2O

2) Cobalt(II) chloride hexahydrate 3) Mercury(II) nitrate monohydrate Practice 1) Beryllium hydroxide octahydrate 2) Cobalt(II) chloride hexahydrate 3) Mercury(II) nitrate monohydrate 4) Tin(IV) chloride pentahydrate

Naming & Identifying Acids All acids contain hydrogen When acids are dissolved in water, H+ ions are generated Acids that generate a lot of H+ are strong acids Acids that generate only a small amount of H+ are weak acids

Strong Acids HCl is a strong acid because no HCl molecules are in a water solution of HCl. Because of the strong attraction between the water molecules and HCl molecules, every HCl molecule ionizes.

Naming & Identifying Acids Cont. The formula for an acid is: HX Where X = an anion

Naming Binary Acids Naming Acids: 1. Begin with the regular name Example HCl is Hydrogen Chloride 2. If the anion ends is “-ide,” add “hydro” as a prefix 3. Replace “-ide” with “-ic”and add acid Example: HCl Hydrogen chloride becomes hydrochloric acid NOTE: It is only an acid with the ending ends in aqueous. If the compound is either gas, liquid, or solid it is not an acid, it is the normal compound.

Name the following binary acids Answers: 1. Hydrofluoric Acid 2. Hydrobromic Acid 3. Hydroiodic Acid 1. HF 2. HBr 3. HI

Naming Ternary Acids Ternary acids contain polyatomic ions To name acids (with 3 or more different elements): 1. Determine regular name of the compound 2. If the anion end in “-ite,” add “-ous” in place of “-ite” and add acid to the end 3. If the anion ends in “-ate,” add “-ic” in place of “-ate” and add acid to the end

Examples of Naming Ternary Acids 1. H2SO3 Name: Hydrogen Sulfite Name of Acid: Sulfurous Acid 2. HNO3 Name: Hydrogen Nitrate Name of Acid: Nitric Acid Begin 3rd 4-28

Name the following ternary acids 1. H3PO4 2. H2CO3 3. H3PO3

Write formulas for the following acids: 1. Chlorous Acid 2. Acetic Acid

Warm Up Write the name or formula of the following Mg(ClO4)2 Copper(II)nitrite Na3(PO4) Cu(OH)

Covalent Bonds Covalent Bonds occur when electrons are shared between atoms Covalent Bonds occur between nonmetals and nonmetals Examples of Covalent Compounds: H2O, SO2, CCl4

Covalent Compounds are molecular compound A molecular compound is composed of only NONMETALS Examples of molecular compounds CO SF6 H2O

Determine if each of the following are molecular compounds 1. CCl4 2. CaCl2 3. Fe2O3 4. P2O5 5. PCl3 6. NH3 7. NaCl

Naming Binary Molecular Compounds Molecular compounds are named using prefixes You will only use prefixes when TWO NONMETALS are involved

Prefixes and Meaning Mono Di Tri Tetra Penta 1 atom 2 atoms 3 atoms 4 atoms 5 atoms

Prefixes and Meaning Hexa Hepta Octa Nona Deca 6 atoms 7 atoms 8 atoms 9 atoms 10 atoms

Naming Molecular Compounds With Molecular compounds, use Greek prefixes The second atom still add “-ide” to its name NOTE: If the first element is a single element you do not have to use a prefix. If the second element is a single element you MUST use a prefix

Naming Molecular Compounds Example: P2O5 SiCl4 CCl4

Write the correct formula for the following nitrogen monoxide carbon disulfide dinitrogen trioxide sodium nitrate aluminum oxide diboron tetrahydride boron monocarbide

Warm-Up Name or write the following Compounds 1) Sodium Acetate 2) MnO2 3) H3PO4 4) Hydrobromic Acid 5) Calcium Sulfate Pentahydrate 6) disulfur trihydride 7) CH4

Practice: Name or write out the following compounds 1. Se2Cl7 2. KMnO4 4 H2O 3. Tetracarbon hexasulfide 4. Al(OH)3 5. Pentanitrogen hexaoxide

Name the following compounds 1. SF6 2. N2O5 3. SO3 4. N2O3 5. NaCl

Practice Write the correct name for the following MnO4 • 3 H2O PH3 SO3 SnO HCl(aq) Li2S H2SO4 (aq)

Name the following or write out the following formulas 1) Carbon tetrachloride 6) NF3 2) Sulfur difluoride 7) S4N4 3) SiO2 8) Silicon tetrachloride 4) ClF4 9) Chlorine trifluoride 5) SeO2 10) Fe(OH)3

Review: Determine the number of Valence electrons for the following Br Sr Pb Fr P Rn

Dot Structures –Lewis structure Dot Structures show the distribution of valence electrons around the nucleus Rules: 1) Determine number of valence electrons 2) Write chemical symbol 3) Place valence electrons in each of the four directions (north, east, south, & west)

5) Pair up electrons once there is one in each of the four directions Dot Structures 4) Distribute one valence electron at a time Do not pair (double up) any electrons until there is one electron in each of the four directions 5) Pair up electrons once there is one in each of the four directions

Example – Dot Structure for O Step 1: O has 6 valence electrons Step 2: Write chemical Symbol O

Example – Dot Structure for O Step 3: Place valence electrons in each of the four directions (north, east, south, & west) This is the correct answer!!! Double up electrons now O = e- Place one in each direction first

Examples for you Write Dot Structures for: 1) H 2) Ne 3) P 4) Ca 5) Al

Hydrogen Answer H Note: You can place the electron in any direction you like when you have less than 4 electrons

Ne Answer Ne

P Answer P

Ca Answer Ca

Al Answer Al

Practice Determine the number of valence electron and draw the dot structure for the following 1) Rb 2) I 3) Te 4) Bi 5) Ra 6) Cl 7) S

Types of Covalent Bonds There are three types of covalent bonds: single, double, triple Single Bonds- result when only 1 pair of electrons are shared

Types of Covalent Bonds H H H

Double Bonds A double bond involves two pairs of electrons being shared

Double Bonds Is when two electrons are being shared

Triple Bonds Triple Bonds result when 3 pairs of electrons are shared N N N

Writing Lewis Dot Structures In writing Lewis structures for covalent compounds, you must remember the following: 1. Determine the total number of valence electrons 2. The least electronegative element goes in the center H is NEVER a center atom Carbon is usually in the center

Writing Lewis Structures 3. Distribute 8 electrons around central atom 4. Place remaining atoms outside of central atom 5. Distribute any remaining electrons around outer atoms

Writing Lewis Structures 6. Use double or triple bonds to obey Octet Rule as needed 7. Check to make sure that every atom obeys the Octet Rule

Write Lewis Dot Structures for the following: 1. H2O 2. CO2 3. NH3 4. CBr4 5. SO2

Practice Draw the Lewis Structures for the Following: 1) GeF4 2) COS 3) SeO3 4) HOF

Practice Draw the following Lewis Structures a. CH4 b. SCl2 c. HCN

Write Lewis structures for the following compounds: 1. H2S 6. NCl3 On Your Own (In Notes): Write Lewis structures for the following compounds: 1. H2S 6. NCl3 2. PH3 7. HCl 3. ClF 8. CS2 4. NF3 9. SeF2 5. N2S

Practice Write Lewis structures for the following molecules: a. HCN d. PH3 b. CHCl3 e. SiO2 c. SeF2 f. CF4